Advertisements
Advertisements
प्रश्न
2500 cm3 of hydrogen is taken at STP. The pressure of this gas is further increased by two and a half times (temperature remaining constant). What volume will hydrogen occupy now?
Advertisements
उत्तर
V1 = 2500 cm3
P1 = 1 atm = 760 mm
T1 = 273 K
V2= ?
T2 = 273 K
`"P"_2 = 760 xx 5/2 + 760 = 1900 + 760 = 2660 "mm"`
`("P"_1 "V"_1)/"T"_1 = ("P"_2 "V"_2)/"T"_2`
`(760xx2500)/273 = (2660xx"V"_2)/273`
`"V"_2 = 5000/7 = 714.29 "cm"^3`
APPEARS IN
संबंधित प्रश्न
Give the assumptions of the kinetic molecular theory.
Explain Charles's law on the basis of the kinetic theory of matter.
State the law which is represented by the following graph:
How did Charles's law lead to the concept of an absolute scale of temperature?
Choose the correct answer:
The volume-temperature relationship is given by
88 cm3 of nitrogen is at a pressure of 770 mm mercury. If the pressure is raised to 880 mmHg, find by how much the volume will diminish, the temperature remaining constant.
An LPG cylinder can withstand a pressure of 14.9 atmospheres. The pressure gauge of the cylinder indicates 12 atmospheres at 27°C. Because of a sudden fire in the building, the temperature rises. At what temperature will the cylinder explode?
State Charles's law.
Give its
(i) graphical representation,
(ii) mathematical expression
(iii) significance
The pressure on one mole of gas at s.t.p. is doubled and the temperature is raised to 546 K. What is the final volume of the gas ? [one mole of a gas occupies a volume of 22.4 litres at stp.]
